A Series of Lanthanide Coordination Polymers as Luminescent Sensors for Selective Detection of Inorganic Ions and Nitrobenzene

Seven new lanthanide coordination polymers, namely [Ln(cpt)3H2O)]n(Ln = La (1), Pr (2), Sm (3), Eu (4), Gd (5), Dy (6), and Er (7)), which were synthesized under hydrothermal conditions using 4′-(4-(4-carboxyphenyloxy)phenyl)-4,2′:6′,4′-tripyridine (Hcpt) as the ligand. The crystal structures of these seven complexes were determined using single-crystal X-ray diffraction, and they were found to be isostructural, crystallizing in the triclinic P1- space group. The Ln(III) ions were nine-coordinated with tricapped trigonal prism coordination geometry. The Ln(III) cations were coordinated by carboxylic and pyridine groups from (cpt)− ligands, forming one-dimensional ring-chain structures. Furthermore, the luminescent properties of complexes 1–7 were investigated using fluorescent spectra in the solid state. The fluorescence sensing experiments demonstrated that complex 4 exhibits high selectivity and sensitivity for detecting Co2+, Cu2+ ions, and nitrobenzene. Moreover, complex 3 shows good capability for detecting Cu2+ ions and nitrobenzene. Additionally, the sensing mechanism was also thoroughly examined through theoretical calculations.


Introduction
With the continuous development of industry and human social activities, a significant amount of heavy metal ions and toxic small molecules are being discharged into our living environment, leading to serious environmental and public health issues [1][2][3][4][5].The sensing and detection of metal ions play a crucial role in environmental and ecological systems, with direct implications for human health and daily life.In biological systems, the Cu 2+ ion is essential, and its imbalance may be associated with metabolic disorders such as Parkinson's, Wilson's, and Alzheimer's [6][7][8][9][10][11]. On the other hand, Co 2+ has toxic effects and can lead to serious health problems including cardiomyopathy, hypothyroidism, peripheral neuropathy, and respiratory disorders [12][13][14].Meanwhile, nitrobenzene (NB), a toxic industrial chemical used as a precursor for explosives, pesticides, and synthetic rubbers and in the production of dyes and pharmaceuticals, poses significant safety risks [15].Furthermore, NB can be easily inhaled, ingested, and absorbed through the skin, leading to methemoglobinemia, hemolytic anemia, splenic congestion, and disorders of the central nervous system (CNS) [16][17][18].Therefore, researchers are dedicated to exploring simple and practical methods for detecting low concentrations of Co 2+ , Cu 2+ , and NB.However, the majority of testing methods require costly instruments and skilled technicians.Therefore, it remains crucial for the protection of the environment and human health to develop efficient methods and design multifunctional materials with high sensitivity and selectivity for detecting Co 2+ , Cu 2+ , and NB.
In recent years, there has been significant attention on the design and construction of lanthanide coordination polymers (Ln-Cps) as luminescent sensors due to their intriguing architectures, high sensitivity, excellent selectivity, rapid response time, and cost effectiveness [19][20][21].The Ln-Cps have been widely reported as luminescent sensors for the detection of anions [22][23][24][25], cations [26], biological molecules [27] and organic molecules [28,29].The 4f orbitals in lanthanide ions are shielded by the filled 5p 6 6s 2 subshells, leading to unique optical properties.Lanthanide coordination polymers exhibit high color purity, narrow band emission, long lifetime, and high quantum yields [30].However, the absorption coefficients and luminescence intensities of pure rare-earth ions are significantly low, and the 4f-4f transitions of lanthanide are Laporte-forbidden.To mitigate these limitations, organic ligands with suitable chromophores can be selected to absorb Uv-vis light and transfer excitation energy from the ligands to lanthanide ions through an "antenna effect", thereby shielding Ln(III) ions from vibrational coupling that dampens luminescence [31].The selection of a suitable ligand is crucial for the construction of lanthanide coordination polymers skeletons, as it determines the structure and chemical environment of the resulting complexes.Choosing long and flexible ligands can contribute to the production of interesting topologies and rich properties.After considering all the aforementioned factors, we chose 4 ′ -(4-(4-carboxyphenoxy)phenyl)-4,2 ′ :6 ′ ,4 ′′ -tripyridine as the ligand based on the following considerations: (1) The Hcpt ligand contains abundant coordination sites, including the nitrogen atom in pyridine and the oxygen atoms of carboxylic acid, all of which can form strong bonds with lanthanide ions and exhibit variable coordination patterns in self-assembly.(2) In addition to the tripyridine and carboxylic group, the Hcpt ligand also contains a phenoxy group, which increases the length and rigidity of the ligand.(3) The Hcpt ligand contains a large π-conjugated system, enabling efficient energy transfer to the lanthanide center for indirect excitation and light emission during relaxation.Additionally, it enhances the thermal stability of lanthanide complexes.(4) To the best of our knowledge, the coordination chemistry and structural properties based on the Hcpt ligand have not been previously reported.

Structural Description of Complexes 1-7
The structures of complexes 1-7 are isostructural; therefore, only the detailed description of complex 4 is provided.The single-crystal X-ray analysis revealed that complex 4 exhibits a one-dimensional ring-chain structure.The asymmetric unit of 4 contains one Eu(III) cation, four (cpt) − ligands, and a water molecule.The coordination polyhedron around Eu(III) is a nine-coordinated dodecahedron consisting of seven oxygen (O 1 , O 1 A, O 7 , O 6 , O 8 , O 4 , and O 10 ) atoms and one nitrogen (N 4 ) from four (cpt) − ligands as well as one oxygen (O 2 ) from one coordinated water molecule (Figure 1a).The Eu-O bond lengths fall within the range of 2.4090(19) Å-2.725(2) Å, while the Eu-N bond lengths are 2.715(2) Å, demonstrating strong consistency with previous research findings [32].
to another atom Eu(III) (Scheme 1b).The Eu(III) atoms are linked by (cpt) − ligands in the two coordination modes, resulting in the formation of a 1D infinite ring-chain structure (Figure 1b).Furthermore, these adjacent chains are further connected via hydrogen bonding interactions between coordinated O atoms and N atoms of (cpt) − ligand (O2-H2B…N2, 2.728 Å), resulting in the formation of a 2D supramolecular structure (Figure 1c).The crystallographic refinement parameters are provided in Tables S1 and S2.(a) It is worth noting that the (cpt) − anion adopts two different coordination fashions: (a) a bidentate coordination fashion in which the carboxylic group acts as a bidentate chelating coordination mode, and the terpyridyl moiety is free (Scheme 1a), and (b) a tridentate coordination fashion in which the carboxylic acid adopts µ 2 -η 1 :η 2 coordination mode, and the terpyridyl moiety acts as the monodentate-chelating coordination mode, coordinating to another atom Eu(III) (Scheme 1b).The Eu(III) atoms are linked by (cpt) − ligands in the two coordination modes, resulting in the formation of a 1D infinite ringchain structure (Figure 1b).Furthermore, these adjacent chains are further connected via hydrogen bonding interactions between coordinated O atoms and N atoms of (cpt) − ligand (O 2 -H 2 B. ..N 2 , 2.728 Å), resulting in the formation of a 2D supramolecular structure (Figure 1c).The crystallographic refinement parameters are provided in Tables S1 and S2.

Luminescent Properties
The solid-state luminescent behaviors of the free ligand and complexes 1-7 were analyzed at ambient temperature when excited at 390 nm.The fluorescence emission of the free ligand was at 474 nm (Figure S1a).For complex 4, the three sharp characteristic peaks shown in Figure 2a belong to the transitions of 5 D0→ 7 F1 (586 nm), 5 D0→ 7 F2 (624 nm), and 5 D0→ 7 F4 (704 nm).The intensity of the 5 D0→ 7 F2 transition (electric dipole) was stronger than that of 5 D0→ 7 F1 transition (magnetic dipole), indicating an asymmetric coordination environment for the Eu 3+ ion, as confirmed by crystallographic analyses.For complex 3, only one characteristic emission band of the Sm(III) cation could be observed in the emission spectra (Figure 2b), which was attributed to 4 G5/2→ 6 H9/2 (680 nm).For complex 6, the

Luminescent Properties
The solid-state luminescent behaviors of the free ligand and complexes 1-7 were analyzed at ambient temperature when excited at 390 nm.The fluorescence emission of the free ligand was at 474 nm (Figure S1a).For complex 4, the three sharp characteristic peaks shown in Figure 2a belong to the transitions of 5 D 0 → 7 F 1 (586 nm), 5 D 0 → 7 F 2 (624 nm), and 5 D 0 → 7 F 4 (704 nm).The intensity of the 5 D 0 → 7 F 2 transition (electric dipole) was stronger than that of 5 D 0 → 7 F 1 transition (magnetic dipole), indicating an asymmetric coordination environment for the Eu 3+ ion, as confirmed by crystallographic analyses.For complex 3, only one characteristic emission band of the Sm(III) cation could be observed in the emission spectra (Figure 2b), which was attributed to 4 G 5/2 → 6 H 9/2 (680 nm).For complex 6, the emission spectra (Figure 2c) revealed the presence of one weak characteristic emission band of the Dy(III) cation, which could be attributed to 4 F 9/2 → 6 H 13/2 (572 nm) transitions.Compared with the emission spectra of the three complexes, the energy transfers from the ligand to Eu(III) were more efficient than those to Sm(III) and Dy(III).The complexes 1, 2, 5, and 7 displayed the characteristic emission peaks of the ligand at 409 nm (1), 450 nm (2), 456 nm (5), and 436 nm (7), all exhibiting a blue shift compared to the free ligand (Figure S1b-e).
Furthermore, the fluorescence lifetime of coordination polymers 4 and 3 were monitored at 624 nm and 680 nm, respectively.The fluorescence decays of the coordination polymers 4 and 3 in the solid state at ambient temperature were fitted into double-exponential decay laws with the following formula: I = A 1 exp(t/τ 1 )+ A 2 exp(t/τ 2 ), where τ 1 and τ 2 are defined as the fast and slow components of the luminescence lifetimes, while A 1 and A 2 denote the preexponential factors (Figure 3).The fitted fluorescence lifetimes τ 1 and τ 2 were 1.15 ns (21.98%) and 4.52 ns (78.02%) for 4 and 1.05 ns (34.10 %) and 4.60 ns (65.90%) for 3.As a result, the average decay times (τ*) was determined by the following equation: , giving the corresponding average lifetimes of 3.78 ns and 3.39 ns.The CIE chromaticity coordinates of the corresponding samples were (0.7309, 0.2691) for complex 4 and (0.1400, 0.0495) for complex 3, as illustrated in Figure 4.

Detection of Metal Ions
The structures of complexes 1-7 are isostructural, and they show a gradual decrease in ionic radius with increasing atomic number (also known as the lanthanide contraction); the resulting applications determine to a large extent these lanthanide ions themselves [33,34].Studies on luminescent lanthanides have concentrated on Sm(III), Eu(III), Tb(III), and Dy(III) ions in the visible region [35], and due to their relatively excellent fluorescence properties, complexes 4 and 3 were selected for investigating their selective sensing behavior towards metal ions.Finely ground samples of 4/3 were suspended in equal volumes of different DMF solutions, each containing a concentration of 1.0 × 10 −2 mol/L of specific M(NO3)n species (M = Li + , Pb 2+ , Mn 2+ , Co 2+ , K + , Na + , Cu 2+ , Cd 2 +, and Zn 2+ ), for luminescence studies at ambient temperature.As shown in Figure 5a,b, the fluorescence emission intensity of complex 4 was most significantly affected by Cu 2+ and Co 2+ ions, showing a more pronounced decrease compared to other ions.The distinct sensing behavior on Cu 2+ and Co 2+ from other cations showed that complex 4 may be employed as an efficient sensor to distinguish Cu 2+ and Co 2+ ions.Interestingly, the luminescence intensity of 3 was quenched close to 0 by only Cu 2+ ions (Figure 6a,b), suggesting that complex 3 can effectively detect Cu 2+ through the phenomenon of fluorescence quenching.
In order to further evaluate the sensitivity of complex 4 in sensing Cu 2+ and Co 2+ as well as the sensing sensitivity of 3 towards Cu 2+ , concentration gradient experiments were conducted with Cu 2+ and Co 2+ concentrations ranging from 10 to 100 µM.The emission

Detection of Metal Ions
The structures of complexes 1-7 are isostructural, and they show a gradual decrease in ionic radius with increasing atomic number (also known as the lanthanide contraction); the resulting applications determine to a large extent these lanthanide ions themselves [33,34].Studies on luminescent lanthanides have concentrated on Sm(III), Eu(III), Tb(III), and Dy(III) ions in the visible region [35], and due to their relatively excellent fluorescence properties, complexes 4 and 3 were selected for investigating their selective sensing behavior towards metal ions.Finely ground samples of 4/3 were suspended in equal volumes of different DMF solutions, each containing a concentration of 1.0 × 10 −2 mol/L of specific M(NO 3 )n species (M = Li + , Pb 2+ , Mn 2+ , Co 2+ , K + , Na + , Cu 2+ , Cd 2 +, and Zn 2+ ), for luminescence studies at ambient temperature.As shown in Figure 5a,b, the fluorescence emission intensity of complex 4 was most significantly affected by Cu 2+ and Co 2+ ions, showing a more pronounced decrease compared to other ions.The distinct sensing behavior on Cu 2+ and Co 2+ from other cations showed that complex 4 may be employed as an efficient sensor to distinguish Cu 2+ and Co 2+ ions.Interestingly, the luminescence intensity of 3 was quenched close to 0 by only Cu 2+ ions (Figure 6a,b), suggesting that complex 3 can effectively detect Cu 2+ through the phenomenon of fluorescence quenching.

Sensing of Organic Small Molecules
The rapid and sensitive detection of toxic small molecules is crucial due to their high toxicity, which poses a potential threat to environmental safety, public health, and human security.After being inspired by this concept, we evaluated the sensing behaviors of complexes 4 and 3 towards various organic small molecules using fluorescence, with the addition of different organic solvents such as CH3CN, NB, CH3CH2OH, CH3OH, DMA, DMF, DMSO, and CH2Cl2 to the suspensions of 4/3.As illustrated in Figures 7a,b   In order to further evaluate the sensitivity of complex 4 in sensing Cu 2+ and Co 2+ as well as the sensing sensitivity of 3 towards Cu 2+ , concentration gradient experiments were conducted with Cu 2+ and Co 2+ concentrations ranging from 10 to 100 µM.The emission intensity of 4 and 3 gradually decreased as the concentration of Co 2+ /Cu 2+ and Cu 2+ increased, as demonstrated in Figure 5c,e and Figure 6c.The fluorescence intensity of complex 4 shows a good linear relationship with ion concentration (R 2 = 0.994 for Cu 2+ and 0.996 for Co 2+ ) in Figure 5d,f.Additionally, the fluorescence intensity of complex 3 demonstrates a good linear relationship with the concentration of Cu 2+ (R 2 = 0.989) in Figure 6d.Furthermore, the quenching efficiency (K sv ) can be quantitatively calculated using the Stern-Volmer equation: I 0 /I = 1 + K sv [M], where I 0 and I represent the emission intensities of the reference sample and complexes, respectively, and [M] represents the concentration [36,37].The K sv values for complex 4 towards Cu 2+ and Co 2+ were calculated to be 4.9 × 10 4 M −1 and 9.4 × 10 4 M −1 , respectively, while the Ksv values for complex 3 towards Cu 2+ were calculated to be 3.53 × 10 4 M −1 .The limit of detection (LOD) was further calculated according to 3σ/k (σ is the standard deviation of 10 blank tests; k is the slope of the linear relationship), which were 8.13 × 10 −5 mol/L for Cu 2+ , 4.4 × 10 −5 mol/L for Co 2+ , and 1.13 × 10 −5 mol/L for Cu 2+ .These values are consistent with those reported for some complex sensors designed to detect Co 2+ and Cu 2+ [38,39].

Sensing of Organic Small Molecules
The rapid and sensitive detection of toxic small molecules is crucial due to their high toxicity, which poses a potential threat to environmental safety, public health, and human security.After being inspired by this concept, we evaluated the sensing behaviors of complexes 4 and 3 towards various organic small molecules using fluorescence, with the addition of different organic solvents such as CH 3 CN, NB, CH 3 CH 2 OH, CH 3 OH, DMA, DMF, DMSO, and CH 2 Cl 2 to the suspensions of 4/3.As illustrated in Figures 7a,b and 8a,b, different degrees of fluorescence intensity quenching were observed for 4 and 3 upon the addition of all selected analytes.Among them, only NB thoroughly quenched the emission of complexes 4 and 3, with a quenching efficiency of approximately 99%.The luminescence of coordination polymers 4 and 3 was significantly influenced by the presence of solvent molecules.Specifically, the CH 3 CN suspension of 4 exhibited the strongest emission band, while the DMF suspension of 3 exhibited the strongest emission band at ambient temperature.Thus, fluorescent detection experiments were performed in CH 3 CN solution of complex 4 and DMF solution of complex 3. To further investigate the sensitivity of fluorescence quenching characteristics for NB, the emissive response was recorded by gradually increasing the concentration of NB in the suspension of coordination polymer 4 dispersed in CH 3 CN and 3 dispersed in DMF.As shown in Figures 7c and 8c, the fluorescence bursting phenomenon of complex 4 was most pronounced at a concentration of 700 ppm NB, with a fluorescence bursting efficiency reaching 99.99%.For complex 3, at a concentration of 1000 ppm NB, the quench efficiency reached as high as 99.99%.Although there is no strict systematic trend in the Figures 7c and 8c, the general trend is still that the quenching effect increases with the increase of concentration, indicating that 4 and 3 are sensitive in detecting trace quantities of NB.

PXRD and FT-IR
To confirm the purities of the bulk samples, PXRD experiments were carried out for lanthanide coordination polymers 1-7 (Figure S2).By comparing the PXRD experimental spectrum of the complex with the theoretical spectrum obtained from fitting single-crystal data, it was observed that the diffraction peak positions in both spectra were essentially consistent.Additionally, no extra diffraction peaks were observed in the experimental spectrum, confirming the purity of the complex obtained.The difference in diffraction peak intensity between the experimental and theoretical spectra can be attributed to the uneven orientation distribution of the powder sample during the diffraction experiment.Moreover, PXRD patterns of complexes 4 and 3 after sensing tests were measured, which are in good agreement with the synthesized 4 and 3, suggesting that the host skeleton remains unchanged after immersion in aqueous solution containing different metal ions (Figure S3).Besides that, the FT-IR spectra of the recycled complexes 4 and 3 were also recorded.And these infrared spectra after processing were highly matched to those before treatment (Figure S4).This indicates that the structure of the complexes 4 and 3 did not collapse during fluorescence detection, and the detected complexes can be recycled for subsequent experiments.
rescence bursting phenomenon of complex 4 was most pronounced at a concentration of 700 ppm NB, with a fluorescence bursting efficiency reaching 99.99%.For complex 3, at a concentration of 1000 ppm NB, the quench efficiency reached as high as 99.99%.Although there is no strict systematic trend in the Figures 7c and 8c, the general trend is still that the quenching effect increases with the increase of concentration, indicating that 4 and 3 are sensitive in detecting trace quantities of NB.

Theoretical Studies
In order to explain the high selectivity and sensitivity of complexes 4 and 3 towards NB, an investigation into the mechanism of fluorescence quenching was conducted.It is well known that fluorescence quenching occurs through mechanisms such as photoinduced electron transfer, long-range energy transfer processes, dynamic-static quenching mechanisms, or a combination of them.The lack of porosity in complexes 4 and 3 excludes the mechanisms of guest-induced fluorescence quenching.The observed fluorescence quenching phenomenon can be attributed to the photoinduced electron transfer from the excited state of the two compounds to the electron-deficient NB, which belongs to the surface adsorption.The coordination polymers can be considered as giant "molecules", and their valence-band (VB) and conduction-band (CB) energy levels can be described in a fashion similar to that used for molecular orbitals (MOs) .The low-lying π* orbitals of nitrobenzene, which are the lowest unoccupied MOs (LUMOs), are stabilized by the -NO 2 substituent.Their orbital energies always fall below the conduction band (CB) of coordination polymers.This leads to the driving force for electron transfer from the coordination polymers to nitrobenzene, thus resulting in fluorescence quenching.Figure 9 exhibits the highest occupied molecular orbital (HOMO) and lowest unoccupied molecular orbital (LUMO) energy levels of ligand and the selected analytes, including NB, as deter-mined through density functional theory (DFT) calculations using the B3LYP/6-31 + G(d) level of theory with the Gaussian 03 package.The LUMO energy of the electron-rich ligand was calculated to be −2.31eV, which is higher than that of NB (−2.92 eV) and lower than those of other tested analytes, indicating that there are excited-state electrons transferred from electron-rich coordination polymers to electron-deficient NB [63,64].

PXRD and FT-IR
To confirm the purities of the bulk samples, PXRD experiments were carried out for lanthanide coordination polymers 1-7 (Figure S2).By comparing the PXRD experimental spectrum of the complex with the theoretical spectrum obtained from fitting single-crystal data, it was observed that the diffraction peak positions in both spectra were essentially consistent.Additionally, no extra diffraction peaks were observed in the experimental spectrum, confirming the purity of the complex obtained.The difference in diffraction peak intensity between the experimental and theoretical spectra can be attributed to the uneven orientation distribution of the powder sample during the diffraction experiment.Moreover, PXRD patterns of complexes 4 and 3 after sensing tests were measured, which are in good agreement with the synthesized 4 and 3, suggesting that the host skeleton remains unchanged after immersion in aqueous solution containing different metal ions (Figure S3).Besides that, the FT-IR spectra of the recycled complexes 4 and 3 were also recorded.And these infrared spectra after processing were highly matched to those before treatment (Figure S4).This indicates that the structure of the complexes 4 and 3 did not The fluorescence of complex 4 and complex 3 results from the antenna effect, in which the Hcpt ligand adsorbs energy through vibronic coupling with Ln 3+ and subsequently transfers this energy to Ln 3+ , resulting in the fluorescence of Ln 3+ .The quenching efficiency of NB may be attributed to the competition for absorption of the light source energy between NB and the Hcpt ligand.NB acts as a filter for the light adsorbed by the Hcpt ligand, thus decreasing the probability of energy transfer from Hcpt to Ln 3+ , consequently leading to the quenching of the fluorescence of the complexes.Therefore, compared to other organic solvents, complexes 4 and 3 exhibit much higher fluorescence quenching responses towards NB due to favorable electron and energy transfer mechanisms.
transfers this energy to Ln 3+ , resulting in the fluorescence of Ln 3+ .The quenching efficiency of NB may be attributed to the competition for absorption of the light source energy between NB and the Hcpt ligand.NB acts as a filter for the light adsorbed by the Hcpt ligand, thus decreasing the probability of energy transfer from Hcpt to Ln 3+ , consequently leading to the quenching of the fluorescence of the complexes.Therefore, compared to other organic solvents, complexes 4 and 3 exhibit much higher fluorescence quenching responses towards NB due to favorable electron and energy transfer mechanisms.

Hirshfeld Surface Analysis
To analyze the various interactions corresponding to the crystal structures, the Hirshfeld surface and 2D fingerprints plot of the complexes 1-7 were calculated based on the crystallographic information file (CIF) using the CrystalExplorer program (Figures 10 and S5).The Hirshfeld surface analysis of complex 4 is described in detail due to the isostructural nature of complexes 1-7.As illustrated in Figure 10, the colors red, white, and blue correspond to the relationship between forces present at that location and the sum of the van der Waals radii [65].The 2D fingerprints of the complexes provide a clearer visualization of the interactions between corresponding atoms (Figure 11).The H. ..H inter-atomic contacts make the most significant contribution to the crystal packing of complex 4 (36.3%).This finding can be attributed to the predominance of hydrogen atoms in the crystal.The H. ..C interaction located in the second ladder contributes to 14% of the complex, while the H. ..O exposure accounts for 4.2%.In addition to these interaction forces, the H. ..N interactions also contribute 4.4% of the total Hirshfeld surface area among all interactions, attributed to the presence of coordinated nitrogen atoms in the complex.In comparison, the H. ..H interaction contributes the most to the structures of the complex.In summary, four forces significantly contributed to the construction and stabilization of molecular structures [66].

Hirshfeld Surface Analysis
To analyze the various interactions corresponding to the crystal structures, the Hirshfeld surface and 2D fingerprints plot of the complexes 1-7 were calculated based on the crystallographic information file (CIF) using the CrystalExplorer program (Figures 10  and S5).The Hirshfeld surface analysis of complex 4 is described in detail due to the isostructural nature of complexes 1-7.As illustrated in Figure 10, the colors red, white, and blue correspond to the relationship between forces present at that location and the sum of the van der Waals radii [65].The 2D fingerprints of the complexes provide a clearer visualization of the interactions between corresponding atoms (Figure 11).The H…H inter-atomic contacts make the most significant contribution to the crystal packing of complex 4 (36.3%).This finding can be attributed to the predominance of hydrogen atoms in the crystal.The H…C interaction located in the second ladder contributes to 14% of the complex, while the H…O exposure accounts for 4.2%.In addition to these interaction forces, the H…N interactions also contribute 4.4% of the total Hirshfeld surface area among all interactions, attributed to the presence of coordinated nitrogen atoms in the complex.In comparison, the H…H interaction contributes the most to the structures of the complex.In summary, four forces significantly contributed to the construction and stabilization of molecular structures [66].

Materials and General Method
All chemicals and reagents were purchased commercially and used without further purification.Infrared spectra were recorded on a Bruker EQUINOX55 spectrometer (Billerica, MA, USA) as KBr pellets in the range of 4000-500 cm −1 .Fluorescence spectra were performed on a Hitachi F-4500 fluorescence spectrophotometer (Tokyo, Japan) at room temperature.The crystal structure was measured using a BRUKER SMART APEX-ⅡCCD X-ray single-crystal diffractometer.Powder X-ray diffraction (PXRD) patterns were recorded on a Bruker D8 Advance instrument with Cu Kα radiation (λ = 0.71073 Å) in the range of 2θ = 5-50° at room temperature.

Synthesis of Complexes
Synthesis of [La(cpt)3(H2O)] (1).A mixture of the ligand Hcpt (22.2 mg, 0.05 mmol) and La(NO3)3•6H2O (43.30 mg, 0.10 mmol) was prepared by dissolving in 10 mL of distilled water; the mixture was stirred at room temperature for 30 min before being transferred into a 25 mL Teflon-lined stainless steel autoclave and heated to 180 °C for 72 h.The reaction system was gradually cooled to ambient temperature at a rate of 5 °C/h, resulting in the formation of colorless, block-shaped crystals of complex 1 in ca.67.33% based on La.Elemental analysis (%) calculated forC84H56LaN9O10 (M = 1490.

Materials and General Method
All chemicals and reagents were purchased commercially and used without further purification.Infrared spectra were recorded on a Bruker EQUINOX55 spectrometer (Billerica, MA, USA) as KBr pellets in the range of 4000-500 cm −1 .Fluorescence spectra were performed on a Hitachi F-4500 fluorescence spectrophotometer (Tokyo, Japan) at room temperature.The crystal structure was measured using a BRUKER SMART APEX-IICCD X-ray single-crystal diffractometer.Powder X-ray diffraction (PXRD) patterns were recorded on a Bruker D8 Advance instrument with Cu Kα radiation (λ = 0.71073 Å) in the range of 2θ = 5-50 • at room temperature.

Synthesis of [La(cpt) 3 (H 2 O)] (1).
A mixture of the ligand Hcpt (22.2 mg, 0.05 mmol) and La(NO 3 ) 3 •6H 2 O (43.30 mg, 0.10 mmol) was prepared by dissolving in 10 mL of distilled water; the mixture was stirred at room temperature for 30 min before being transferred into a 25 mL Teflon-lined stainless steel autoclave and heated to 180 • C for 72 h.The reaction system was gradually cooled to ambient temperature at a rate of 5

X-ray Crystallography
We selected a single crystal with a clean and smooth surface, no concave surface, and no cracks.At the temperature of 293(2) K, we used a BRUKER SMART APEX-IICCD X-ray single crystal diffractometer and graphite monochromatic Mo-Kα (λ = 0.71073 Å) rays, and diffraction data were collected in ω-φ scanning.All data were corrected by empirical absorption, and the crystal structure was solved using the direct method.The anisotropy parameters and the coordinates of all non-hydrogen atoms were corrected using the least squares method.F 2 was refined using the SHELXTL-97 program, and the hydrogen atoms were obtained by theoretical calculation methods.Crystallographic data and experimental details of structural analyses for complexes are summarized in Table S1.The selected bond length and angle parameters are listed in Table S2.

Conclusions
In conclusion, after hydrothermal synthesis, seven new Lanthanide coordination polymers, namely [Ln(cpt) 3 H 2 O)]n(Ln = La (1), Pr (2), Sm (3), Eu (4), Gd (5), Dy (6), and Er (7)), were successfully obtained.Remarkably, complex 4 exhibited remarkable sensitivity and selectivity toward Co 2+ , Cu 2+ and nitrobenzene.Complex 3 demonstrated effective detection of Cu 2+ and nitrobenzene through the phenomenon of fluorescence quenching.Furthermore, the mechanism of the high selectivity and sensitivity of complex 4 and 3 for NB were also investigated by theoretical studies.The two coordination polymers exhibited much higher fluorescence quenching responses towards NB due to favorable electron and energy transfer mechanisms.The work presented in this study offers valuable insights for the development of sensitive fluorescent recognition sensors with multifunctional applications.
Crystallographic data for the structural analysis were deposited with the Cambridge Crystallographic Data Center, CCDC reference numbers: 2283726 for complex 1, 2283709 for complex 2, 2283707 for complex 3, 2283701 for complex 4, 2283708 for complex 5, 2328935 for complex 6, and 2283727 for complex 7.These data can be obtained free of charge from The Cambridge Crystallographic Data Centre via www.ccdc.cam.ac.uk/data_request/cif (accessed on 17 June 2024).

Figure 1 .
Figure 1.(a) Coordination environment of the Eu III cations in complex 4. (b) The one-dimensional ring-chain structure of complex 4. (c) Two-dimensional supramolecular structure of complex 4.

Figure 1 .
Figure 1.(a) Coordination environment of the Eu III cations in complex 4. (b) The one-dimensional ring-chain structure of complex 4. (c) Two-dimensional supramolecular structure of complex 4.

Figure 1 .Scheme 1 .
Figure 1.(a) Coordination environment of the Eu III cations in complex 4. (b) The one-dimensional ring-chain structure of complex 4. (c) Two-dimensional supramolecular structure of complex 4.

Figure 5 .Figure 5 .Figure 6 .
Figure 5. (a) Emission spectra of complex 4 in diverse metal ions.(b) Comparisons for intensities of complex 4 in different metal ions.(c,e) Luminescence quenching of complex 4 dispersed in DMF Figure 5. (a) Emission spectra of complex 4 in diverse metal ions.(b) Comparisons for intensities of complex 4 in different metal ions.(c,e) Luminescence quenching of complex 4 dispersed in DMF with gradual addition of Cu 2+ and Co 2+ ions, respectively.(d,f) The fitting of the fluorescence change value of complex 4 in Cu 2+ and Co 2+ ions, respectively.
and 8a,b, different degrees of fluorescence intensity quenching were observed for 4 and 3 upon the

Figure 6 .
Figure 6.(a) Emission spectra of complex 3 in diverse metal ions.(b) Comparisons for intensities of complex 3 in different metal ions.(c) Luminescence quenching of complex 3 dispersed in DMF with gradual addition of Cu 2+ ion.(d) The fitting of the fluorescence change value of complex 3 in Cu 2+ ion.

Figure 7 .
Figure 7. (a) Emission spectra of complex 4 in diverse analytes.(b) Comparisons for intensities of 4 in diverse analytes.(c) Emission spectra of complex 4 in CH3CN with different concentrations of NB.

Figure 7 .
Figure 7. (a) Emission spectra of complex 4 in diverse analytes.(b) Comparisons for intensities of 4 in diverse analytes.(c) Emission spectra of complex 4 in CH 3 CN with different concentrations of NB.

Figure 8 .
Figure 8.(a) Emission spectra of complex 3 in diverse analytes.(b) Comparisons for intensities of 3 in diverse analytes.(c) Emission spectra of complex 3 in DMF with different concentrations of NB.

Figure 8 .
Figure 8.(a) Emission spectra of complex 3 in diverse analytes.(b) Comparisons for intensities of 3 in diverse analytes.(c) Emission spectra of complex 3 in DMF with different concentrations of NB.

Figure 9 .
Figure 9. HOMO and LUMO energy levels of ligand and the selected analytes.

Figure 9 .
Figure 9. HOMO and LUMO energy levels of ligand and the selected analytes.